Scientists determine the quantity of atmospheric sulfur dioxide ( SO2 ), a large contributor to acid rain, by an indirect titration. First, a scientist collects a sample of air and reacts it with hydrogen peroxide ( H2O2 ) to form a solution of sulfuric acid ( H2SO4 ). Then, the amount of H2SO4 produced is determined by titration with a sodium hydroxide solution ( NaOH ) of known concentration. H2O2(aq)+SO2(g)⟶H2SO4(aq) H2SO4(aq)+2NaOH(aq)⟶2H2O(l)+Na2SO4( aq) Suppose Lane collects a 658.0 g sample of air that is known to contain SO2 and reacts it with excess H2O2 . A volume of 22.4 mL of 0.025 M NaOH is required to neutralize the H2SO4 produced. Calculate the mass percent of SO2 in the air sample.

the solar system used to have much dust particles option no d

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole

i believe the answer is 5,000

yes the answer is total mass in unchanged   : )